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Chapter 7: Problem 61

Discuss the similarities and differences between a \(1 s\) and a \(2 s\) orbital.

Short Answer

Expert verified
The 1s and 2s orbitals are both s-type orbitals, spherical and hold up to 2 electrons. Differences are that the 2s orbital is at a higher energy level, is larger, and has one radial node, while the 1s orbital has no nodes.

Step by step solution

01

Define an s orbital

An s orbital is the simplest type of atomic orbital. It is spherical in shape and is centered around the nucleus of the atom. The 's' stands for sharp.
02

Discuss the 1s Orbital

A 1s orbital is the first, and thus closest, energy level to the nucleus. It is the smallest in size, and can hold up to 2 electrons. The distribution of the electron cloud is uniform and it does not have any node (a region where there is a zero probability of finding an electron) within it.
03

Discuss the 2s Orbital

A 2s orbital is at the second energy level. It is larger than the 1s orbital, indicating that the electrons in this orbital are usually found further from the nucleus compared to the 1s orbital. The 2s orbital can also hold up to 2 electrons. However, unlike the 1s orbital, the 2s orbital has one radial node.
04

Similarities and Differences

The similarities between the 1s and 2s orbitals include: both are s-type orbitals, both are spherical in shape and both can each contain 2 electrons. The main differences between the 1s and the 2s orbitals lie in their size, energy, and the presence of a node. The 2s is larger, has more energy and a radial node, unlike the 1s orbital that has no nodes.

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Most popular questions from this chapter

What are the inadequacies of Bohr's theory?

What is an atomic orbital? How does an atomic orbital differ from an orbit?

For each of the following pairs of hydrogen orbitals, indicate which is higher in energy: (a) \(1 s, 2 s ;\) (b) \(2 p\) \(3 p ;\) (c) \(3 d_{x y}, 3 d_{y c}\) (d) \(3 s, 3 d ;\) (e) \(4 f, 5 s\)

In the beginning of the twentieth century, some scientists thought that a nucleus may contain both electrons and protons. Use the Heisenberg uncertainty principle to show that an electron cannot be confined within a nucleus. Repeat the calculation for a proton. Comment on your results. Assume the radius of a nucleus to be \(1.0 \times 10^{-15} \mathrm{~m} .\) The masses of an electron and a proton are \(9.109 \times 10^{-31} \mathrm{~kg}\) and \(1.673 \times 10^{-27} \mathrm{~kg},\) respectively. (Hint: Treat the diameter of the nucleus as the uncertainty in position.)

Atoms of an element have only two accessible excited states. In an emission experiment, however, three spectral lines were observed. Explain. Write an equation relating the shortest wavelength to the other two wavelengths.
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